Basics

Question 1

What is the charge and mass of a proton?

Answer 1

Charge= +1
Mass= 1

Question 2

What is the charge and mass of a neutron?

Answer 2

Charge= 0
Mass= 1

Question 3

What is the charge and mass of an electron?

Answer 3

Charge= -1
Mass= 0

Question 4

What did Dalton say about the Billiard Ball?

Answer 4

That atoms were solid spheres and different spheres made up different elements

Question 5

What was JJ Thompson atom model called?

Answer 5

The plum pudding model which said that atoms were positive spheres with negative electrons

Question 6

What did Ernest Ruthford create that we use today?

Answer 6

The planetary model
Added shells and a positively charged nucleus

Question 7

What are Isotopes?

Answer 7

Different forms of the same element which have the same number of protons but different number of neutrons

Question 8

Due to Isotopes having the same of protons but different number of neutrons what does this suggest?

Answer 8

The atomic number is constant but the mass number changes

Question 9

What does it mean if an element has only one isotope?

Answer 9

The mass number is the same as the abundance

Question 10

What does it mean if an element has more than one isotope?

Answer 10

You must take into account how much of each one there is (find the average of the mass number of all the isotopes)

Question 11

What is the relative atomic mass?

Answer 11

An average mass of all the isotopes of an element

Question 12

What are the steps for when you’re asked to calculate the relative atomic mass of copper?

Answer 12

1. Times the mass by the abundance percentage for all the isotopes mentioned
2. Add them together
3. Divide it all by 100

Question 13

What is Ionic Bonding?

Answer 13

Bonds between a metal and non-metal

Question 14

Why do atoms bond to get a full outer shell?

Answer 14

Because if they don’t have a full outer shell they are NOT stable

Question 15

What is an ion?

Answer 15

A charged particle

Question 16

How is an ion formed?

Answer 16

By the loss or gain of electrons

Question 17

What happens to electrons when atoms form ionic bonds?

Answer 17

They either loose or gain electrons

Question 18

What with the charge of an element be if it looses one electron?

Answer 18

+1 as it lost negative charge becoming a cation

Question 19

What is the charge of an element if it gains 1 electron?

Answer 19

-1 as it gained negative charge becoming a anion

Question 20

What is the name of the structure that Ionic compounds form?

Answer 20

Giant Crystal Lattice

Question 21

(Example is same for all) For sodium chloride (salt) how will the ions be arranged in a giant crystal lattice?

Answer 21

The Na+ and Cl- ions are will alternate (same for any ionic bond)

Question 22

What holds the ions together in a giant crystal lattice?

Answer 22

Strong electrostatic forces between the positive and negative ions

Question 23

What are electrostatic forces?

Answer 23

Strong forces between positive and negative ions

Question 24

Can ionic compounds conduct electricity as a solid and why or why not?

Answer 24

Ionic compounds CAN’T conduct electricity when a solid as ions are fixed in place

Question 25

What do you have to do to ionic compounds to make them conduct electricity and why?

Answer 25

They must be dissolved into or molten to conduct electricity as when they are the ions are free to move and will conduct an electrical current

Question 26

Why do ionic compounds have high melting and boiling points?

Answer 26

Ionic compounds have high melting and boiling points as you need lots of energy to overcome the strong electrostatic forces between ions

Question 27

When doing ionic equations what are the two important steps to remember?

Answer 27

1. Split into ions 2. Remove ions that don’t change in the equation

Question 28

When does covalent bonding occur?

Answer 28

Occurs when two non-metal atoms share electrons to achieve a full outer shell

Question 29

What is between the non metal atoms in a covalent bond?

Answer 29

Strong covalent bonds

Question 30

What is between the whole covalent molecules themselves?

Answer 30

Weak intermolecular forces

Question 31

In ionic bonding what does a metal always become?

Answer 31

A positive ion/ cation

Question 32

In ionic bonding what does the non-metal always become?

Answer 32

A negative ion/ anion

Question 33

Why do covalent molecules have low melting and boiling points?

Answer 33

The weak intermolecular forces between molecules are easily overcome. (They become a gas easily)

Question 34

What are the two different types of giant covalent structures?

Answer 34

-Diamond -Graphite

Question 35

What are the features of the giant covalent structure Diamond?

Answer 35

-made from a network of carbon atoms that each form four covalent bonds -high melting points as a lot of energy is needed to break strong covalent bonds -atoms are in rigid lattice structure meaning it is hard and strong (used for tools) -Doesn’t conduct electricity as there is no free electron to delocalise and conduct a current

Question 36

What are the features of the giant covalent structure graphite?

Answer 36

-only forms three covalent bonds creating sheets of carbon atoms in hexagons -organised in layers making it soft and a lubricating metal -high melting points as covalent bonds are strong and need a lot of energy to break -only 3 out of 4 electrons are used in covalent bonds so 1 electron is free to delocalise and conduct a current (Can conduct electricity used for electrodes)